6K + Al2O3 🔥→ 3K2O + 2Al
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- Reaction of and aluminium oxide
The reaction of and aluminium oxide yields potassium oxide and . This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of and aluminium oxide
General equation
- Reaction of reducing species and hardly reducible species
- Reducing speciesReducing agent + Hardly reducible speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of and aluminium oxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 6 | Reducing | Reducing | ||
| Al2O3 | Aluminium oxide | 1 | Oxidizing | Hardly reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K2O | Potassium oxide | 3 | Oxidized | – |
| 2 | Reduced | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of and aluminium oxide◆
ΔrG 616.0 kJ/mol K 0.12 × 10−107 pK 107.92
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | 591.2 | 616.0 | −97.0 | 43.3 |
| 98.53 | 102.7 | −16.2 | 7.22 | |
per 1 mol of | 591.2 | 616.0 | −97.0 | 43.3 |
per 1 mol of | 197.1 | 205.3 | −32.3 | 14.4 |
| 295.6 | 308.0 | −48.5 | 21.6 |
Changes in standard condition (2)
- Reaction of and aluminium oxide
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | 582.0 | – | – | – |
| 97.00 | – | – | – | |
per 1 mol of | 582.0 | – | – | – |
per 1 mol of | 194.0 | – | – | – |
| 291.0 | – | – | – |
Changes in standard condition (3)
- Reaction of and aluminium oxide
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | 573 | – | – | – |
| 95.5 | – | – | – | |
per 1 mol of | 573 | – | – | – |
per 1 mol of | 191 | – | – | – |
| 287 | – | – | – |
Changes in standard condition (4)
- Reaction of and aluminium oxide
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | 577.8 | – | – | – |
| 96.30 | – | – | – | |
per 1 mol of | 577.8 | – | – | – |
per 1 mol of | 192.6 | – | – | – |
| 288.9 | – | – | – |
Changes in standard condition (5)
- Reaction of and aluminium oxide
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | 572.4 | – | – | – |
| 95.40 | – | – | – | |
per 1 mol of | 572.4 | – | – | – |
per 1 mol of | 190.8 | – | – | – |
| 286.2 | – | – | – |
Changes in standard condition (6)
- Reaction of and aluminium oxide
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | 548 | – | – | – |
| 91.3 | – | – | – | |
per 1 mol of | 548 | – | – | – |
per 1 mol of | 183 | – | – | – |
| 274 | – | – | – |
Changes in aqueous solution
- Reaction of and aluminium oxide◆
ΔrG 616.0 kJ/mol K 0.12 × 10−107 pK 107.92
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | 591.2 | 616.0 | −97.0 | 43.3 |
| 98.53 | 102.7 | −16.2 | 7.22 | |
per 1 mol of | 591.2 | 616.0 | −97.0 | 43.3 |
per 1 mol of | 197.1 | 205.3 | −32.3 | 14.4 |
| 295.6 | 308.0 | −48.5 | 21.6 |
Thermodynamic data of reactants
| Chemical formula | Standard enthalpy of formation ΔfH° kJ · mol−1 | Standard Gibbs energy of formation ΔfG° kJ · mol−1 | Standard molar entropy S° J · K−1 · mol−1 | Standard molar heat capacity at constant pressure Cp° J · K−1 · mol−1 |
|---|---|---|---|---|
| (cr) | 0[1] | 0[1] | 64.18[1] | 29.58[1] |
| (g) | 89.24[1] | 60.59[1] | 160.336[1] | 20.786[1] |
| Al2O3 (cr) α, corundum | -1675.7[1] | -1582.3[1] | 50.92[1] | 79.04[1] |
| Al2O3 (cr) δ | -1666.5[1] | – | – | – |
| Al2O3 (cr) ρ | -1657[1] | – | – | – |
| Al2O3 (cr) κ | -1662.3[1] | – | – | – |
| Al2O3 (cr) γ | -1656.9[1] | – | – | – |
| Al2O3 (am) | -1632[1] | – | – | – |
| Al2O3 (cr) 1 hydrate | -1998.91[1] | -1841.78[1] | 70.67[1] | 106.19[1] |
| Al2O3 (cr) 3 hydrate | -2576.5[1] | – | – | – |
* (cr):Crystalline solid, (g):Gas, (am):Amorphous solid
Thermodynamic data of products
| Chemical formula | Standard enthalpy of formation ΔfH° kJ · mol−1 | Standard Gibbs energy of formation ΔfG° kJ · mol−1 | Standard molar entropy S° J · K−1 · mol−1 | Standard molar heat capacity at constant pressure Cp° J · K−1 · mol−1 |
|---|---|---|---|---|
| K2O (cr) | -361.5[1] | -322.1[2] | 94.1[2] | 83.7[2] |
| K2O (g) | -63[1] | – | – | – |
| (cr) | 0[1] | 0[1] | 28.33[1] | 24.35[1] |
| (g) | 326.4[1] | 285.7[1] | 164.54[1] | 21.38[1] |
* (cr):Crystalline solid, (g):Gas
References
List of references
- 1Janiel J. Reed (1989)The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI UnitsNational Institute of Standards and Technology (NIST)
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 64.18 J · K−1 · mol−1
- ^ Cp°, 29.58 J · K−1 · mol−1
- ^ ΔfH°, 89.24 kJ · mol−1
- ^ ΔfG°, 60.59 kJ · mol−1
- ^ S°, 160.336 J · K−1 · mol−1
- ^ Cp°, 20.786 J · K−1 · mol−1
- ^ ΔfH°, -1675.7 kJ · mol−1
- ^ ΔfG°, -1582.3 kJ · mol−1
- ^ S°, 50.92 J · K−1 · mol−1
- ^ Cp°, 79.04 J · K−1 · mol−1
- ^ ΔfH°, -1666.5 kJ · mol−1
- ^ ΔfH°, -1657. kJ · mol−1
- ^ ΔfH°, -1662.3 kJ · mol−1
- ^ ΔfH°, -1656.9 kJ · mol−1
- ^ ΔfH°, -1632. kJ · mol−1
- ^ ΔfH°, -1998.91 kJ · mol−1
- ^ ΔfG°, -1841.78 kJ · mol−1
- ^ S°, 70.67 J · K−1 · mol−1
- ^ Cp°, 106.19 J · K−1 · mol−1
- ^ ΔfH°, -2576.5 kJ · mol−1
- ^ ΔfH°, -361.5 kJ · mol−1
- ^ ΔfH°, -63. kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 28.33 J · K−1 · mol−1
- ^ Cp°, 24.35 J · K−1 · mol−1
- ^ ΔfH°, 326.4 kJ · mol−1
- ^ ΔfG°, 285.7 kJ · mol−1
- ^ S°, 164.54 J · K−1 · mol−1
- ^ Cp°, 21.38 J · K−1 · mol−1
- 2James G. Speight (2017)Lange's Handbook of Chemistry, 17th editionMcGraw Hill Education
- ^ ΔfG°, -322.1 kJ · mol−1 - p.280
- ^ S°, 94.1 J · K−1 · mol−1 - p.280
- ^ Cp°, 83.7 J · K−1 · mol−1 - p.280